Polarity of Bond
Polarity of Bond
The
existence of a hundred percent ionic or covalent bond represents an ideal
situation. In reality no bond or a compound is either completely covalent or
ionic. Even in case of covalent bond between two hydrogen atoms, there is some
ionic character.
When
covalent bond is formed between two similar atoms, for example in H2,
O2, Cl2 N2 or F2, the shared pair
of electrons is equally attracted by the two atoms. as a result electron pair
is situated exactly between the two identical nuclei. The bond so formed is
called nonpolar covalent bond. Contrary to this in case of a heteronuclear
molecule like HF, the shared electron pair between the two atoms gets displaced
more towards fluorine since the electronegativity of fluorine is far greater
than that of hydrogen. The resultant covalent bond is a polar covalent bond.
As a result
of polarization, the molecule possesses the dipole moment (depicted
below) which can be defined as the product of the magnitude of the charge and
the distance between the centres of positive and negative charge. It is usually
designated by a Greek latter ‘ ‘. Mathematically, it is expressed as follows:
Dipole
Moment (μ) = charge (Q) distance of separation (r)
Dipole
moment is usually expressed in Debye units (D).
The conversion factor is
1D =
3.33564 10-30 Cm, where C is coulomb and m is meter.
Further
dipole moment is a vector quantity and is depicted by a small arrow with tail
on the positive centre and head pointing towards the negative centre. For
example the dipole moment of HF may be represented as:
The shift in
electron density is symbolized by crossed arrow above the Lewis structure to
indicate the direction of the shift.
In case of
polyatomic molecules the dipole moments not only depend upon the individual
dipole moments of bonds known as bond dipoles but also on the spatial
arrangement of various bonds in the molecule. In such case, the dipole moment
of a molecule is the vector sum of the dipole moments of various bonds. For
example in H2O molecule, which has a bent structure, the two O-H
bonds are oriented at an angle of 104.5o. Net dipole moment of
6.17 10-30C m
(1D=3.33564 10-30 C m) is the
resultant of the dipole moments of two O-H
bonds.
Net Dipole
moment, = 1.85 D = 1.85
3.33564 10-30 C m =
6.17 10-30 C m
The dipole
moment in case of BeF2 is zero. This is because the two equal bond dipoles
point in opposite directions and cancel the effect of each other.
In
tetra-atomic molecule, for example in BF3, the dipole moment is zero although
the B – F bonds are oriented at an angle of 120o to one another, the
three bond moments give a net sum of zero as the resultant of any two is equal
and opposite to the third.
Let us study
an interesting case of NH3 and NF3 electrons on nitrogen atom. Although fluorine is more
electronegative than nitrogen, the resultant dipole moment of NH3(4.90 10-30 C m) is greater than that
of NF3 (0.8 10-30 C m). This
is because, in case of NH3 the orbital dipole due to lone pair is in the same
direction as the resultant dipole moment of the N – H bonds, whereas in NF3 the
orbital dipole is in the direction opposite to the resultant dipole moment of
the three N –F bond moments, which results in the low dipole moment of NF3 as
represented below :
Just as
all the covalent bonds have some partial ionic character, the ionic bonds also
have partial covalent character. The partial covalent character of ionic bonds
was discussed by Fajans in terms of the following rules:
The smaller
the size of the cation and the larger the size of the anion, the greater the
covalent character of an ionic bond.
The greater
the charge on the cation, the greater the covalent character of the ionic bond.
For cations
of the same size and charge, the one, with electronic configuration
(n-1)dnnso, typical of
transition metals, is more polarising than the one with a noble gas
configuration, ns2 np6, typical of alkali and alkaline earth metal cations.
The cation
polarizes the anion, pulling the electronic charge towards itself and thereby
increasing the electronic charge between the two. This is precisely what
happens in a covalent bond, i.e., buildup of electron charge density between
the nuclei. The polarizing power of the cation, the polarisability of the anion
and the extent of distortion (polarization) of anion are the factors, which determine
the per cent covalent character of the ionic bond.
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